Calculate the value of the equilibrium constant (Kc) for the reaction shown, if SbCl5 was found to be 5.57% decomposed at 521K when its initial concentration was 7.60M.
SbCl5 <==> SbCl3 + Cl2
4 answers
Assume the chlorine gas is dissolved in the same volume of solution.
K=122
I am assuming that these are solutions, somehow, but the equation you have shown doesn't tell me what they are. At 521 K I suspect we have a gaseous reaction. The reason I'm a little puzzled is that these probably are in the gaseous state, and the problem wants you to calculate Kp first, then change to Kc. Until I get clarification, I'll assume concns but I would be willing to bet good money that they are gases initially.
Write the decomposition equation.
Write the Kc expression.
Set up an ICE chart if that will help you.
Calculate concns SbCl5, SbCl3, and Cl2.
For example, the equilibrium concn of Cl2 will be 0.0557 x 7.60 M= ??
Write the decomposition equation.
Write the Kc expression.
Set up an ICE chart if that will help you.
Calculate concns SbCl5, SbCl3, and Cl2.
For example, the equilibrium concn of Cl2 will be 0.0557 x 7.60 M= ??
oh sorry, all of them are in gaseous states
1 answer